By using the following data draw an appropriate enthalpy cycle & Calculate the enthalpy change of hydration of (i) the chloride ion , (ii) the iodide ion.
Comment on the difference in their values.
`{:(**,,"enthalpy change of solution of "NaCl(s)=-2" kJ/mol."),(**,,"enthalpy change of solution of "NaI(s)=+2" kJ/mol."),(**,,"enthalpy change of hydration of "Na^(+)(g)=-390" kJ/mol."),(**,,"lattice anthalpy of "NaCl=-772" kJ/mol."),(**,,"lattice enthalpy of "NaI=-699" kJ/mol."):}`

Answer

for `Cl^(-) -384" kJ mol"^(-1)`, for `I^(-) -307" kJ mol"^(-1)`

Explanation

(i) `-2=722-390+x` [Where x= Ethalpy change of hydration of iodine ion]
`x=-384" kJ mol"^(-1)`
(ii) `2=699-390+x" "`[x= Ethalpy change of hydration of iodide ion]
`x=-307" kJ mol"^(-1)`